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Electro-chemistry: Batteries and plating

Electrochemistry : The study of the interchange of chemical and electrical energy Oxidation i s the l oss of electrons (Increase in charge). OIL Reduction i s the g ain of electrons (Decrease in charge) RIG. Electro-chemistry: Batteries and plating. Can you make electricity with chemicals?.

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Electro-chemistry: Batteries and plating

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  1. Electrochemistry: The study of the interchange of chemical and electrical energy Oxidationis the loss of electrons (Increase in charge). OIL Reductionis the gain of electrons (Decrease in charge) RIG Electro-chemistry: Batteries and plating

  2. Can you make electricity with chemicals? You need: 2 metals and 2 solutions of the same metal (ions) The more active metal will LOSE electrons to the less active metal (it’s ions) which will GAIN Electrons

  3. Electrochemical Cells: Device capable of either generating electrical energy from chemical reactions or facilitating chemical reactions through the introduction of electrical energy • Voltaic Cells: • Produces electrical current • spontaneous chemical reactions •  ex. Battery • 2. Electrolytic Cells • Consumes electrical current • non-spontaneous and require electricity or battery •  ex. Electrolysis, electroplating

  4. Parts of the voltaic cell… Anode  the electrode where oxidation occurs After a period of time, the anode may appear to become smaller as it falls into solution. Cathode  the electrode where reduction occurs After a period of time it may appear larger, due to ions from solution plating onto it. Salt Bridge  a device used to maintain electrical neutrality in a voltaic cell. This may be filled with a salt solution. Electron Flow  always from anode to cathode (through the wire) Ion Flow  always through the salt bridge

  5. Cathode Anode

  6. VOLTAIC CELLS (also called electrochemical cells) 2 or more cells = a battery Electricitycan be made from a spontaneous redox reaction, instead of heat, light ... measured in volts 2 half cells 1 side loses electrons to the other side that gains The more active metal looses, higher on Chart J Cu+2 + 2e- Cu0 Zn0 Zn+2 + 2e- - ions flow in salt bridge e-’s flows on wire GER LEO anode cathode Copper metal Zinc metal Cu solution like CuSO4(aq) Zn solution like ZnSO4 (aq) “ Dead” battery has reached equilibrium, volts = 0

  7. ELECTROLYTIC CELLS Redox reactions that are not spontaneous andrequire electricity Electrolysis: splitting a chemical apart into its elements using electricity H2O  H2 (g) + O2 (g) + + battery H + + 1 e- H 0 H2O GER (cathode) O-2O 0 + 2e- LEO (anode)

  8. Also an Electrolytic cell (Requires electricity or a battery) Electroplating: adding a layer of a metal onto another metal (usually expensive metals onto cheaper metal) - + battery - fork to be plated - solution with metal ions - - metal for plating Ag+ Ag Ag+ + 1e- Ag0 Ag0 Ag+1 + 1 e- reduction oxidation anode cathode

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